Answer:
The answer to your question is Pressure = 3.55 atm
Explanation:
Data
R = 0.082 atm L/mol°K
mass = 4.5 g
volume = 2 L
temperature = 35°C
Pressure = ?
Process
1.- Calculate the moles of Methane
molar weight = 12 + 4 = 16 g
16 g of Methane --------------- 1 mol
4.5 g --------------- x
x = (4.5 x 1)/16
x = 0.281 moles
2.- Convert temperature to Kelvin
°K = 273 + 35
= 308
3.- Use the ideal gas law to solve this problem
PV = nRT
- Solve for P
P = nRT / V
- Substitution
P = (0.281)(0.082)(308) / 2
- Simplification
P = 7.097 / 2
- Result
P = 3.55 atm
Answer:
The pressure in the container is 3.55 atm
Explanation:
Step 1: Data given
Mass of methane gas = 4.50 grams
Volume = 2.00 L
Temperature = 35 °C = 308 K
Molar mass CH4 = 16.04 g/mol
Step 2: Calculate moles CH4
Moles CH4 = mass CH4 / molar mass CH4
Moles CH4 = 4.50 grams / 16.04 g/mol
Moles CH4 = 0.281 moles
Step 3: Calculate pressure
p*V = n*R*T
⇒with p = the pressure in the container = TO BE DETERMINED
⇒with V = the volume of the container = 2.00L
⇒with n = the moles of methane = 0.281 moles
⇒with R = the gas constant = 0.08206 L*atm/mol*K
⇒ T = the temperature = 308 K
p = (n*R*T)/V
p = (0.281 * 0.08206 * 308 ) / 2.00
p = 3.55 atm
The pressure in the container is 3.55 atm
